The ka of a monoprotic weak acid is 6.07 × 10-3. what is the percent ionization of a 0.179 m solution of this acid?

What you need to do my friend is write the chemical equation of dissociation of your acid AH with water, with initial concentration co, then consider that a fraction α reacts with water. Concentration and Ka are big enough so that you can consider that
1−α≈1
 Then write expression of Ka, then solve for α. You should find about 18.4% I hope this works really good for you

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